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wel
3 years ago
15

Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reac- t

ion vessel contains 11.5 g NH3, 12.0 g O2, and 10.5 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written?
Chemistry
1 answer:
Sliva [168]3 years ago
8 0

Answer:

Mass of HCN produced = 6.75 g

Explanation:

Reaction is as follows:

2NH_3+3O_2+2CH_4 \rightarrow 2HCN + 6H_2O

First calculate the no. of moles of each chemical species.

molecular mass of NH_3 is 17 g/mol

No. of mol of NH_3 = 11.5/17 = 0.676 mol

Molecular mass of O_2 = 32 g/mol

No. of  mol of O_2 = 12/32 = 0.375

Molecular mass of CH_4 = 16 g/mol

No. of  mol of CH_4 = 10.5/16 = 0.656 mol

from the balanced chemical reaction, it is clear that 2-moles ammonia reacts with 3 moles oxygen and 2 moles methane to form 2 moles of HCN.

or, 1-mol ammonia reacts with 1.5 mol oxygen and 1 mol methane to form 1 mol of HCN.

Thus, no. of oxygen present is less than required and so it will act as limiting reagent.

From the chemical equation,

3 moles oxygen produces 2 moles HCN

or one mole oxygen produces (2/3) moles HCN

0.375 moles oxygen produces (2/3) × 0.375 HCN = 0.25 moles of HCN  

molar mass of HCN = 27 g/mole

Mass = mol × molar mass

mass of HCN = 27 × 0.25 = 6.75 g

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from (1)

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